To flip the current card, click it or press the Spacebar key.
To move the current card to one of the three colored boxes, click on the box. You may also
press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to
move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.
You may also click on the card displayed in any of the three boxes to bring that card back to the
center.

Science C2 Topic 1

In a periodic table according to the properties and compounds of elements. He used predicted existence of elements & left gaps for them. Horizontal rows (periods) are arranged by increasing atomic number. Columns (groups) are by common properties

What are the properties (mass, location, charge) of protons, neutrons and electrons?

Electrons: negligible mass, in shells orbitting the nucleus, charge is -1. Neutrons: mass of 1 AMU, found in the nucleus, neutral charge. Protons: mass of 1 AMU, found in nucleus, charge of +1

What is the atomic number and where is this written?

The number of protons, which is equal to the number of electrons- written at the bottom of each cell of the periodic table

What is the mass number and where is this written?

The number of neutrons plus protons- written at the top of each cell of the periodic table

What is an electron configuration?

The number of electrons in each energy level

What is the maximum electron configuration?

2,8,8

What does the electron configuration of an element tell you about the positioning of that element in the periodic table?

Amount of numbers in electron configuration tells you the period (row). The number of electrons in outer shell tells you the group number (column)

What is an isotope?

An atom of a particular element with a different amount of neutrons, meaning it has a different mass number

What is the relative atomic mass and how do you calculate it?

Relative atomic mass is the mass of an atom of an element taking into account the relative abundance of each isotope. RAM = (percentage of isotope X mass number) + (percentage of isotope X mass number)...

Why aren't relative atomic masses always whole numbers?

The presence of isotopes mean numbers have to be added and multiplied etc. producing numbers that aren't always whole